Which of the following pairs of elements in t | vedclass

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(C) Step $1$: Determine the electronic configuration and number of unpaired electrons for each ion.$Fe^{2+}$ $(Z=26)$: $[Ar] 3d^6$. Unpaired electrons

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$Fe^{2+}$ and $Cr^{2+}$

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(C) Step $1$: Determine the electronic configuration and number of unpaired electrons for each ion.$Fe^{2+}$ $(Z=26)$: $[Ar] 3d^6$. Unpaired electrons = $4$.$Mn^{2+}$ $(Z=25)$: $[Ar] 3d^5$. Unpaired electrons = $5$.$Co^{2+}$ $(Z=27)$: $[Ar] 3d^7$. Unpaired electrons = $3$.$Ni^{2+}$ $(Z=28)$: $[Ar] 3d^8$. Unpaired electrons = $2$.$Cr^{2+}$ $(Z=24)$: $[Ar] 3d^4$. Unpaired electrons = $4$.Step $2$: Compare the number of unpaired electrons.$Fe^{2+}$ has $4$ unpaired electrons and $Cr^{2+}$ has $4$ unpaired electrons.Therefore, the pair $Fe^{2+}$ and $Cr^{2+}$ has the same number of unpaired electrons.

List-$I$ (Property)	List-$II$ (Metal)
$(A)$ Element that can show $+8$ oxidation state	$(1)$ $Mn$
$(B)$ $3d$ series element that can show up to $+7$ oxidation state	$(2)$ $Cr$
$(C)$ $3d$ series element with maximum melting point	$(3)$ $Os$
	$(4)$ $Fe$

Which of the following pairs of elements in their respective oxidation states have the same number of unpaired electrons?

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